Functionalized silanes and electrolyte compositions and electrochemical devices containing them

ABSTRACT

Described are compounds of the structure R 4-a —Si-(Sp-Y) a —Z b , wherein “a” is an integer from 1 to 4; “b” is an integer from 0 to (3×a); “Z,” which is absent when “b”=0, is “R” or 
                         
wherein each “R” is halogen, C 1-6  linear or branched alkyl, alkenyl, or alkynyl or C 1-6  linear or branched halo-alkyl, halo-alkenyl, or halo-alkynyl; each “Sp” C 1-15  linear or branched alkylenyl or C 1-15  linear or branched halo-alkylenyl; and each “Y” an organic polar group. Also described are electrolyte compositions containing one or more of these compounds.

CROSS-REFERENCE TO RELATED APPLICATIONS

This is a continuation of application Ser. No. 15/508,279, filed Mar. 2, 2017, now U.S. Pat. No. 10,355,313, issued Jul. 16, 2019, which is a national phase application of PCT/US015/053930, filed Oct. 5, 2015, which claims priority to U.S. provisional application Ser. No. 62/059,663, filed Oct. 3, 2014, all of which are incorporated herein.

BACKGROUND

Liquid electrolytes in Li-ion batteries conventionally comprise a lithium salt, usually LiPF₆, in an organic solvent blend of ethylene carbonate (EC) and one or more co-solvents such as dimethyl carbonate (DMC), diethyl carbonate (DEC), or ethylmethyl carbonate (EMC). Unfortunately, LiPF₆ is unstable in these carbonate solvents above 60° C., as well as at charge voltages above 4.3 volts. Operation of a Li-ion battery above these temperatures or voltages results in rapid degradation of electrode materials and battery performance. In addition, current Li-ion electrolyte solvents exhibit flashpoints around 35° C., and are the major source of the energy released during an extreme Li-ion cell failure. Given these significant limitations, current electrolytes are impeding the development of advanced Li-ion batteries for all uses, including portable products, electric drive vehicles (EDVs), and utility scale use. A dramatic reduction in battery failure rate is also required for large scale Li-ion batteries to effectively serve applications in EDVs and grid storage.

Thus, there is a long-felt and unmet need for improved electrolyte solutions in energy storage devices such as Li-ion batteries.

SUMMARY OF THE INVENTION

Disclosed herein are organosilicon (OS) compounds for use as electrolyte solvents in electrochemical devices, among other uses.

In general, OS compounds are environmentally friendly, non-flammable, high temperature-resistant materials. These characteristics make OS materials well-suited for use as electrolyte solvents, binders, and coatings in energy storage devices. OS-based electrolytes are compatible with all lithium (Li) based electrochemical systems, including primary and rechargeable batteries, (i.e. Li-ion, Li-air), and capacitors (i.e. super/ultra-capacitors). The process of designing OS-based electrolytes into a Li battery involves limited changes in the cell design, and these electrolytes can be incorporated into production operations with existing manufacturing processes and equipment.

The OS compounds described herein can be used as liquid electrolyte solvents that replace the carbonate based solvent system in traditional Li-ion batteries. The OS-based solvents provide significant improvements in performance and abuse tolerance in Li-ion batteries, including increased thermal stability for longer life at elevated temperatures, increased electrolyte flash points for improved safety, increased voltage stability to allow use of high voltage cathode materials and achieve higher energy density, reduced battery failure rates for consistency with the requirements for large scale Li batteries used in EDV and grid storage applications, and compatibility with materials currently in use in Li-ion batteries for ease of adoption in current designs. Electrical double-layer capacitor (EDLC) devices have also demonstrated functionality with OS based electrolytes. The OS compounds described herein can be used in OS-based electrolyte blends to meet the requirements of specific applications in the industrial, military, and consumer product devices.

The objects and advantages of the compounds and electrolyte formulations will appear more fully from the following detailed description and accompanying drawings.

Thus, disclosed herein are:

1. A compound selected from the group consisting of: (R)_(4-a)—Si-(Sp-Y)_(a)—Z_(b)  (Formula I)

wherein:

“a” is an integer from 1 to 4; “b” is an integer from 0 to (3×a);

“Z,” which is absent when “b”=0, is selected from the group consisting of “R” and

where each “R” is independently selected from the group consisting of halogen, C₁₋₆ linear or branched alkyl, alkenyl, or alkynyl and C₁₋₆ linear or branched halo-alkyl, halo-alkenyl, or halo-alkynyl;

each “Sp” in Formulas I and II is independently selected from the group consisting of C₁₋₁₅ linear or branched alkylenyl and C₁₋₁₅ linear or branched halo-alkylenyl; and

each “Y” in Formula I is independently selected from the group consisting of an organic polar group.

2. The compound of Claim 1, wherein each “Y” is independently an organic polar group selected from the group consisting of:

wherein a curved bond denotes a C₂₋₆ alkylene bridging moiety.

3. The compound of Claim 2, wherein each “Y” is independently an organic polar group selected from the group consisting of:

4. The compound of Claim 3, wherein each “R” is independently selected from the group consisting of fluorine and C₁₋₆ linear or branched fluoro-alkyl, fluoro-alkenyl, or fluoro-alkynyl; and

each “Sp” in Formulas I and II is independently selected from the group consisting of C₁₋₁₅ linear or branched fluoro-alkylenyl.

5. The compound of any one of Claims 1-4, wherein “a” is 1, and “b” is 0 to 3.

6. The compound according to Claim 5, wherein “b” is 1 and “Z” is “—R”.

7. The compound according to Claim 5, wherein at least one “R” is fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear alkylene and C₁₋₆ linear fluoro-alkylene.

8. The compound of any one of Claims 1-4, wherein “a” is 2, and “b” is 0 to 6.

9. The compound according to Claim 7, wherein “b” is 1 and “Z” is “R”.

10. The compound according to Claim 7, wherein at least one “R” is fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear alkylene.

11. The compound of any one of Claims 1-4, wherein “a” is 3, and “b” is 0 to 9.

12. The compound according to Claim 11, wherein “b” is 1 and “Z” is “R”.

13. The compound according to Claim 11, wherein at least one “R” is fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear alkylene.

14. The compound of any one of Claims 1-4, wherein “a” is 4, and “b” is 0 to 12.

15. The compound according to Claim 14, wherein “b” is 1 and “Z” is “R”.

16. The compound according to Claim 14, wherein at least one “R” is fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear alkylene.

17. The compound of any one of Claims 1-4, wherein at least one “R” is fluorine.

18. An electrolyte composition comprising a compound as recited in any one of Claims 1-4, in combination with a salt.

19. The electrolyte composition of Claim 18, wherein the salt is a lithium-containing salt.

20. An electrochemical device comprising an electrolyte composition as recited in Claim 18.

In more limited versions of the compounds, each “Y” is independently an organic polar group selected from the group consisting of:

Additionally, each “Y” may optionally and independently be an organic polar group selected from the group consisting of:

In an alternative version of the compounds, “a” is 1, and “b” is 0 to 2; optionally “b” is 1 and “Z” is R. In this version, an optional embodiment is for at least one “R” to be fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear or branched alkylene which could be fluorinated.

In another alternative version of the compounds, “a” is 2, and “b” is 0 to 6; optionally “b” is 1 and “Z” is R. In this version, an optional embodiment is for at least one “R” to be fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear or branched alkylene which could be fluorinated.

In yet another alternative version of the compounds, “a” is 3, and “b” is 0 to 9; optionally “b” is 1 and “Z” is R. In this version, an optional embodiment is for at least one “R” to be fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear or branched alkylene which could be fluorinated.

In still another alternative version of the compounds, “a” is 4, and “b” is 0 to 12; optionally, “b” is 1 and “Z” is R. In this version, an optional embodiment is for at least one “R” to be fluorine, and each “Sp” is independently selected from the group consisting of C₁₋₆ linear or branched alkylene which could be fluorinated.

Also disclosed herein is an electrolyte composition comprising a compound as herein, in combination with a salt. Lithium-containing salts are preferred. Also disclosed herein is an electrochemical device comprising the electrolyte composition.

Due to the nature of the subscripts “a” and “b”, the following generic structures are explicitly within the scope of the compounds disclosed and claimed herein:

The various R groups are as defined above for “R”; Sp is as defined above, Y is as defined above. Preferably, in all versions of the compounds, Y is an organic polar group that can coordinate Li⁺.

When the polar group Y has a valency of two (2) or more it will have more than one site for substitution. Thus, there can be more than one silicon atom bonded to Y through a spacer group, as noted in the definition for Z above. Thus, the following structures are also explicitly within the scope of the compounds disclosed and claimed herein:

etc.

In all versions of the compounds, “halogen,” includes fluoro, chloro, bromo, and iodo. Fluoro and chloro are the preferred halogen substituents. The term “salt” is used herein in its conventional chemical sense to mean ionic compounds that result from the neutralization reaction of an acid and a base. As used herein, salt is purposefully defined broadly to include all salts, including, but not limited to sodium salts, lithium salts, magnesium salts, borate salts, phosphate salts, and the like. Non-limiting examples include sodium hexafluorophosphate, sodium perchlorate, sodium bis-trifluoromethanesulfonimide, magnesium hexafluorophosphate, magnesium perchlorate, magnesium bis-trifluoromethanesulfonimide, magnesium tetrafluoroborate, magnesium trifluoromethyl sulfonate, tetraethylammonium tetrafluoroborate (TEA-TFB), tetrabutylphosphonium tetrafluoroborate, tetrabutylphosphonium hexafluorophosphate, tetrabutylammonium tetrafluoroborate, tetraethylammonium hexafluorophosphate, tetraethylammonium perchlorate, and tetraethylammonium bistrifluoromethanesulfonimidate. The term “lithium-containing salt” explicitly includes, but is not limited to, LiClO₄, LiBF₄, LiAsF₆, LiPF₆, LiCF₃SO₃, Li(CF₃SO₂)₂N, Li(CF₃SO₂)₃C, LiN(SO₂C₂F₅)₂, lithium alkyl fluorophosphates and lithium bis(chelato)borates.

Also disclosed herein are electrolyte compositions comprising one or more organosilicon compounds as recited in the preceding paragraphs. Also disclosed herein are electrochemical devices comprising such electrolyte compositions. The compounds disclosed herein are highly useful for formulating electrolytes for use in charge-storage devices of all kinds (e.g., cells, batteries, capacitors, and the like).

The organosilicon solvent molecules disclosed herein have remarkable and unexpected thermal stability as compared to conventional carbonate solvents. Even when formulated into electrolyte compositions including lithium salts such as LiPF₆, the organosilicon solvents exhibit remarkable resistance to breakdown during high-temperature exposure and operation. As shown in the examples and figures, several variations of the organosilicon solvent molecules disclosed herein have demonstrated thermostability in the presence of LiPF₆ at temperatures up to and exceeding 175° C. These data demonstrate the intrinsic benefit of silicon as an essential stabilizing element within the organosilicon molecular design. Variations of molecules disclosed herein include non-fluorinated, fluorinated, multi-fluorinated, multi-functional, and alternate alkyl structures, as well as many different Li⁺ coordinating functionalities. The functional groups include nitriles, carbonates, sulfones, and esters among many others. Both gas phase and liquid phase decomposition were measured by EI-MS and NMR respectively to determine breakdown of electrolytes with organosilicon solvent plus 1M LiPF₆ salt after exposure to 175° C. for 60 minutes. There was no significant gas or liquid phase decomposition of OS solvents observed.

Numerical ranges as used herein shall include every number and subset of numbers contained within that range, whether specifically disclosed or not. Further, these numerical ranges shall be construed as providing support for a claim directed to any number or subset of numbers in that range. For example, a disclosure of from 1 to 10 shall be construed as supporting a range of from 2 to 8, from 3 to 7, from 1 to 9, from 3.6 to 4.6, from 3.5 to 9.9, and so forth.

All references to singular characteristics or limitations of the present invention shall include the corresponding plural characteristic or limitation, and vice-versa, unless otherwise specified or clearly implied to the contrary by the context in which the reference is made. The indefinite article “a” shall mean “at least one,” unless explicitly limited to the singular.

All combinations of method or process steps as used herein can be performed in any order, unless otherwise specified or clearly implied to the contrary by the context in which the referenced combination is made.

BRIEF DESCRIPTION OF THE DRAWINGS

FIG. 1A depict the oxidation stability of F1S₃MN with LiPF₆, LiBF₄, or LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). FIG. 1B depicts a close-up of the same data shown in FIG. 1A.

FIG. 2A and FIG. 2B depict duplicate runs to measure the reduction stability of F1S₃MN with LiPF₆, LiBF₄, or LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺).

FIG. 3A depicts the oxidation stability of F1S₃MN or F1S₃M2 with 1M LiPF₆ in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). FIG. 3B depicts a close-up of the same data shown in FIG. 3A.

FIG. 4 depicts the reduction stability of F1S₃MN or F1S₃M2 with 1M LiPF₆ in current density (mA/cm²) versus voltage (V vs. Li/Li⁺).

FIGS. 5A and 5B depict the thermal stability of F1S₃MN with LiPF₆. FIG. 5A depicts a close-up of the same data shown in FIG. 5B.

FIG. 6 depicts the thermal stability of F1S₃M2 with LiPF₆.

FIG. 7 depicts the thermal stability of F1S₃MN with LiTFSI.

FIG. 8 depicts the thermal stability of F1S₃MN with LiBF₄.

FIG. 9 depicts the thermal stability of neat F1S₃MN.

FIG. 10 depicts the thermal stability of DF1S₃MN with 20% EC and VC/LiBOB.

FIG. 11 depicts the enhanced stability of F1S₃MN electrolytes compared to carbonate control electrolyte heated with de-lithiated NCA cathode.

FIG. 12 depicts the discharge capacity of cells containing various electrolyte solvents at a variety of C-rates at 30° C.

FIG. 13 depicts the construction of a test cell.

FIG. 14 depicts the discharge capacity of cells containing the same electrolyte solvents shown in FIG. 12 at a variety of C-rates at 55° C.

FIG. 15 depicts the construction of an EDLC device.

FIG. 16 depicts the performance of an EDLC device containing DF1S₂MN electrolyte with TEA-BF₄.

FIG. 17 depicts the performance of an EDLC device containing various electrolyte solvents with TBP-PF₆.

FIG. 18 depicts the oxidation stability of 1ND1N with 1M LiPF₆ or 1M LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺).

FIG. 19 depicts the reduction stability of 1ND1N with 1M LiPF₆ or 1M LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺).

FIGS. 20A and 20B depict current density (mA/cm²) versus voltage (V vs. Li/Li⁺) for cycling scans with 1ND1N and 1M LiPF₆ or 1M LiTFSI from 0 to 6 V and from 6 to 0 V. FIG. 20A depicts a first cycle. FIG. 20B depicts a second cycle.

FIG. 21A depicts the oxidation stability of F1S₃MN or 1ND1N with 1M LiPF₆ in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). FIG. 21B depicts a close-up of the same data shown in FIG. 21A.

FIG. 22A depicts the oxidation stability of F1S₃MN or 1ND1N with 1M LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). FIG. 22B depicts a close-up of the same data shown in FIG. 22A.

FIG. 23 is a mass spectrum illustrating the thermal stability of neat 1ND1N.

FIG. 24 is a mass spectrum illustrating the thermal stability of 1ND1N with LiPF₆.

FIG. 25A depicts a close-up of the mass spectrum profile as described with respect to FIG. 24 from 24-30 m/z. FIG. 25B depicts a close-up of the mass spectrum profile as described with respect to FIG. 24 from 49-55 m/z.

FIG. 26 depicts the thermal stability of 1ND1N with LiTFSI, vinylene carbonate (VC) and lithium bis(oxalato)borate (LiBOB).

FIG. 27 depicts the thermal stability of 1ND1N with LiBF₄.

FIG. 28 depicts the discharge capacity of cells containing various electrolytes at a variety of C-rates.

FIG. 29 depicts the discharge capacity of cells containing various other electrolyte solvents comparing the first cycle to the 50^(th) cycle.

FIG. 30A depicts the discharge capacity of cells containing a 1ND1N-LiPF₆-based electrolyte at a variety of C-rates. FIG. 30B depicts the discharge capacity of cells containing a 1ND1N-LiTFSI-based electrolyte at a variety of C-rates.

FIG. 31 is the ¹H-NMR spectrum (in CDCl₃) of 1ND1N with peak assignments.

FIG. 32 is the ¹H-NMR spectrum (in CDCl₃) of F1S₃MN with peak assignments.

FIG. 33 is the ¹H-NMR spectrum (in CDCl₃) of DF1S₂MN with peak assignments.

FIG. 34 is the ¹H-NMR spectrum (in CDCl₃) of DF1S₃MN with peak assignments.

FIG. 35 is the ¹H-NMR spectrum (in CDCl₃) of F1S₃cMN with peak assignments.

FIG. 36 is the ¹H-NMR spectrum (in CDCl₃) of 1S₃MN with peak assignments.

FIG. 37 depicts the gas phase decomposition of F1S₃MC, F1S₃cMN, and 1S₃DN with 1M LiPF₆ after 60 min at 175° C. The figure shows no significant gas phase decomposition up to 175° C.

FIG. 38 depicts the gas phase decomposition of DF1S₂MN, TF1S₂MN and TF1S₃MN with 1M LiPF₆ after 60 min at 175° C. The figure shows no significant gas phase decomposition up to 175° C.

DETAILED DESCRIPTION OF THE INVENTION

Throughout the description, a number of shorthand abbreviations will be used to designate various organosilicon compounds more easily. The following conventions are used:

The FnSnMN compounds have the general formula:

wherein R¹, R², and R³ are the same or different and are independently selected from the group consisting of C₁ to C₆ linear or branched alkyl, alkenyl, alkynyl, or halogen (preferably F), “spacer” is a C₁ to C₆ linear or branched alkylene (preferably C₁ to C₆ linear divalent alkylene). and Y is a polar organic moiety as described earlier.

The compounds disclosed herein can be made by a number of different routes. A general approach that can be used to fabricate the compounds is as follows:

The R¹, R², and R³ groups are as defined for R herein; R⁴ has the same definition as Y; “n” is a positive integer.

The compounds disclosed herein can also be fabricated via the following approach:

Again, the R¹, R², and R³ groups are as defined for R herein; R⁴ has the same definition as Y.

The compounds disclosed herein are also made by a number of specific routes, including the following reaction schemes:

LiTFSI, bis(trifluoromethane)sulfonimide lithium salt (Sigma-Aldrich catalog no. 449504), is a commercial product supplied by several international suppliers:

The elements and method steps described herein can be used in any combination whether explicitly described or not.

All combinations of method steps as used herein can be performed in any order, unless otherwise specified or clearly implied to the contrary by the context in which the referenced combination is made.

As used herein, the singular forms “a,” “an,” and “the” include plural referents unless the content clearly dictates otherwise.

All patents, patent publications, and peer-reviewed publications (i.e., “references”) cited herein are expressly incorporated by reference to the same extent as if each individual reference were specifically and individually indicated as being incorporated by reference. In case of conflict between the present disclosure and the incorporated references, the present disclosure controls.

It is understood that the compounds and compositions disclosed herein are not confined to the particular construction and arrangement of parts herein illustrated and described, but embraces such modified forms thereof as come within the scope of the claims.

The presently disclosed compounds are organosilicon compounds having a shared structural feature in the form of a one or more terminal or internal polar organic substituents or moieties. As used herein, the term “polar organic substituent” and “polar organic moiety” are used interchangeable. The terms explicitly include, but are not limited to, the following functional groups:

Included among the preferred compounds are the following structures:

The above structures are all depicted with a terminal cyano group. This is for purposes of brevity only. The analogous compounds having internal and/or terminal polar moieties as described above in place of the cyano moiety are explicitly within the scope of the disclosure. Likewise, the halogenated compounds are depicted above as fluorinated compounds. The analogous compounds having other halogen substituents (chlorine, bromine, and/or iodine) in place of fluorine atoms are explicitly within the scope of the present disclosure. For each compound listed, two alternative systematic names are provided (the first of each pair of names designates the fundamental core as a nitrile; the second designated the fundamental cores as silane.) Additionally, each compound has been given a short-hand designation in which DF=difluoro, TF=trifluoro, and “Sn” designates the alkylene spacer between the silicon atom and the terminal cyanate, isocyanate, or thiocyanate moiety and “n” represents the number of carbon atoms in the spacer. The physical properties of selected organosilicon (OS) compounds are presented in Table 1.

The synthesis of the analogous sulfones can be accomplished using the following illustrative synthesis of the compounds designated, 1NMS, F1S₃MS, and DF1S₃MS. Note that other sulfones falling within the broader disclosure contained herein can be made by the same route by simply altering accordingly the starting reagents.

The synthesis of 1NMS proceeded as follows: 2-(Methylsulfonyl)ethanol was mixed with 0.5 mol equivalents of hexamethyldisilazane and about 1% mol equivalents of Al(H₂PO₄)₃ as catalyst, without solvent. The mixture was kept at about 80° C. overnight and distilled twice to get pure 1NMS.

The synthesis of F1S₃MS proceeded as follows: Allylmethylsulfide was dissolved in ethanol and mixed with 4 mol equivalents of H₂O₂. Approximately 3% mol equivalents of ammonium heptamolybdate was added as catalyst for oxidation. The next day the solution was neutralized with NaHCO₃ solution and extracted with CH₂Cl₂, the water fraction was discarded, and the organic layer evaporated and distilled to yield allylmethylsulfone. Allylmethylsulfone was hydrosilylated with dimethylchlorosilane using Karstedt's catalyst. The product was fluorinated using NaFHF at about 150° C., filtered, distilled twice, and dried over a molecular sieve to yield pure F1S₃MS

The synthesis of DF1S₃MS proceeded as follows: 3-mercaptopropylmethyldimethoxysilane was dissolved in ethanol and mixed with one (1) mol equivalent of NaOH in water. One (1) mol equivalent of Me₂SO₄ was then added to the mixture and refluxed overnight. The solid was filtered off. The crude product was oxidized with 4 mol equivalents of H₂O₂ and 3% mol equivalents of ammonium heptamolybdate. The solvent was evaporated and 2 mol equivalents of HF in water was added. The product was extracted with CH₂Cl₂ and distilled.

Additional characterization data for these sulfone compounds is contained in the appendix, attached hereto and incorporated herein.

As shown in Table 1, Reduced viscosity, higher conductivity, and lower flash point with added fluorine and reduced spacer length. DF1S₂MN has lowest viscosity and highest conductivity.

TABLE 1 Physical Properties (with 20% EC, additives, 1M LiPF₆) Electrolyte Properties (w/1M LiPF₆) at 30° C. Neat Solvent Properties No co-solvent 20% EC FP BP Den. Cond. Vis. Cond. Vis. OS MW Diel ° C. ° C. g/mL mS/cm cP mS/cm cP 1S₂MN 127 12.3 52 n/a 0.83 2.6 7.7 n/a n/a 1S₃MN 141 12.6 72 200 0.81 1.6 9.4 Phase Phase sep. sep. with with EC EC F1S₃MN 145 16.8 82 249 0.93 2.8 8.0 4.2 8.5 DF1S₃MN 149 18.2 78 202 1.09 3.5 7.9 4.8 8.3 DF1S₂MN 135 19.5 64 182 1.10 5.0 6.8 5.7 7.6 TF1S₃MN 153 16.7 68 n/a 1.22 3.0 10.2 4.0 9.5 TF1S₂MN 139 n/a 64 n/a 1.30 n/a n/a n/a n/a DPF1S₃MN 201 12.5 118 206 0.91 0.44 43 n/a n/a Key:

 

 

 

 

 

 

 

The physical properties of neat 1ND2, 1ND1, 1ND1N, F1S₃MN, DPF1S₃MN, F1S₃MC, F1S₃ME, F1S₃MA, F1S₃MS, 1NMS, F1S₃M2, and F1S₃cMN as well as electrolyte solutions containing these solvents, are shown in Table 2:

TABLE 2 Physical Properties of Solvents and Electrolytes Electrolyte Properties (w/1M LiPF₆) at 30° C. Neat Solvent Properties No co-solvent 20% EC Flash BP Density Cond. Vis. Cond. Vis. OS MW Diel. ° C. ° C. g/mL mS/cm cP mS/cm cP 1ND2 296 6.4 138 288 1.07 n/a n/a 3.6 12 1ND1 208 8.1 85 n/a 0.94 n/a n/a 4.5 5.1 1ND1N 198 30 168 n/a 1.03 1.3 29 1.9 33 F1S₃MN 145 16.8 82 249 0.93 2.8 8.0 4.2 8.5 DPF1S₃MN 201 12.5 118 206 0.91 0.44 43 n/a n/a F1S₃MC 194 4.9 86 188 1.02 0.62 11.4 2.1 10.5 F1S₃ME 178 6.6 66 170 0.96 1.8 7.2 n/a n/a F1S₃MA 163 4.8 n/a 155 0.85 n/a n/a n/a n/a F1S₃MS 198 29.4 158 245 1.11 0.3 177 1.0 65 1NMS 196 19.6 48 290 1.06 n/a n/a 1.5 37 F1S₃M2 238 7.2 112 233 n/a n/a n/a 3.0 14.0 F1S₃cMN 159 16.6 80 n/a n/a n/a n/a 2.6 10.6 Key:

 

 

 

 

 

 

 

 

 

 

 

In addition to the organosilicon compounds disclosed herein, the present electrolyte compositions may include conventional non-silicon co-solvents. For example, the present electrolyte compositions may include nitriles and carbonates, such as acetonitrile, ethylene carbonate (EC), dimethyl carbonate (DMC), diethyl carbonate (DEC), or ethylmethyl carbonate (EMC). The instant electrolyte compositions may include non-silicon co-solvents at a wide range of concentrations, including but not limited to, about 1 wt % to about 40 wt %. Examples of suitable co-solvent concentrations include about 1 wt %, about 5 wt %, about 10 wt %, about 15 wt %, about 20 wt %, about 25 wt %, about 30 wt %, about 40 wt % or a range between and including any of the preceding amounts.

EXAMPLES

F1S₃MN Synthesis:

Scheme 1 depicts a synthesis scheme for F1S₃MN. [F] indicates a fluorinating agent, such as HF, NH₄FHF, or other fluorinating agent. NH₄FHF is preferably used as a fluorinating agent for laboratory scale synthesis. If HF is used, the only byproduct is HCl. The synthesized F1S₃MN compound is washed from the solid salt with hexane, distilled, dried with CaO, and distilled again.

Scheme 2 depicts a synthesis scheme for F1S₃MN using NH₄FHF as a fluorinating agent. Using Karstedt's catalyst (Platinum(0)-1,3-divinyl-1,1,3,3-tetramethyldisiloxane complex solution, Cat. No. 479519, Sigma-Aldrich, St. Louis, Mo.), about 3% substitution on the secondary carbon occurs, generating isoF1S₃MN. The isoF1S₃MN has a lower boiling point than F1S₃MN, and most of it can be separated by fractional distillation.

Scheme 3 depicts an alternative, shorter synthesis scheme for F1S₃MN using a Cl1S₃MN intermediate. The Cl1S₃MN intermediate can be obtained by Gelest, Inc. (Product Code SIC2452.0, 11 East Steel Road, Morrisville, Pa.). Use of the Cl1S₃MN intermediate reduces the time spent during synthesis.

Scheme 4 depicts yet another synthesis scheme for F1S₃MN. As with Scheme 1, [F] indicates a fluorinating agent, such as HF, NH₄FHF, or other fluorinating agent. The use of HF as fluorinating agent in this synthesis scheme will not give solid byproducts, so there is no need of hexane extraction and filtration of solid. The only byproduct is HCl.

Scheme 5 depicts yet another synthesis scheme for F1S₃MN. As with Scheme 1, [F] indicates a fluorinating agent, such as HF, NH₄FHF, or other fluorinating agent.

Synthesis of F1S₃MN

In the preferred route, allyl cyanide is heated to about 100° C. with a small amount of Karstedt's catalyst. Dimethylchlorosilane was added dropwise and refluxed 4 hours. After cooling to room temperature, the mixture was fluorinated using 1 mol equivalent of ammonium hydrogen fluoride at room temperature. Cold hexane was added to the mixture, the solid was filtered off, and the solvent evaporated. Calcium oxide was added to the crude product and it was distilled under vacuum between 45-55° C. at 0.4 Torr to yield the desired product, F1S₃MN.

Synthesis of F1S₃ME

In the preferred route, allyl acetate is mixed with dimethylchlorosilane and a small amount of Karstedt's catalyst is added. The mixture is left reacting overnight. Next day, the mixture was fluorinated using 0.33 mol equivalent of antimony trifluoride at room temperature overnight with strong stirring. Next day, the solid was filtered off, and the product distilled under vacuum between 25-30° C. at 0.3 Torr to yield the desired product, F1S₃ME.

This ester is suitable as an electrochemical solvent in an electrolyte composition. F1S₃ME has good solubility with 1M LiPF₆ and dissolved readily at room temperature. Its flash point is acceptable at 66° C., as is its dielectric constant of 6.6. Its CV oxidation/reduction behavior is likewise suitable for lithium ion charge storage cells. Full cell cycling with 80% F1S₃ME electrolyte was stable with good capacity. It retained a very low current density at potentials at or below 5 V at 30° C. F1S₃ME is electrochemically viable by fundamental Pt oxidation and graphite reduction. It displayed normal reduction behavior in on the first cycle and passivation was observed on the second cycle. F1S₃ME cycled well in an 80% electrolyte formulation in a NMC/graphite electrode system through 26 cycles (data not shown).

Synthesis of DF1S₃DN

Bis(cyanopropyl)dichlorosilane was mixed with 2 mol equivalents of aqueous HF at room temperature and left reacting overnight. The crude product was extracted with dichloromethane, the solvent evaporated and the product distilled under vacuum at 165° C. at 0.1 Torr to yield the desired product, DF1S₃DN.

Synthesis of 1S₃DN

DF1S₃DN was dissolved in THF and cooled with an ice bath, then 2 mol equivalents of methylmagnesium bromide were added and the mixture was left reacting until it slowly reached room temperature. The mixture was quenched with ethanol, the crude product was extracted with dichloromethane, the solvent evaporated and the product distilled under vacuum at 125° C. at 0.2 Torr to yield the desired product, 1S₃DN.

Synthesis of TF1S₃MN

Cyanopropyltrichlorosilane was cooled in an ice bath and 4 mol equivalents of aqueous HF were added dropwise. The mixture was left reacting no more than 2 hours. The crude product was extracted with dichloromethane, the solvent evaporated and the product distilled under vacuum at 25° C. at 0.2 Torr to yield the desired product, TF1S₃MN.

Synthesis of DPF1S₃MN

Bis(isopropyl)cyanopropylchlorosilane was dissolved in THF and cooled in an ice bath, then 1 mol equivalent of aqueous HF was added dropwise and left reacting overnight at room temperature. Next day the solvent was evaporated and the product distilled under vacuum at 60° C. at 0.2 Torr to yield the desired product, DPF1S₃MN.

DPF1S₃MN was made to explore how larger alkyl groups on the silicon atom impact the physical characteristics and electronic characteristics of the molecule. This compound has good solubility with LiPF₆, dissolving readily at room temperature. It displayed stable oxidation behavior in cyclic voltammetry (CV) up to approximately 5 V. Its CV reduction behavior was also good, with passivation on the second cycle. This compound is suitable for electrochemical applications at elevated temperatures (flash point=118° C.) and at potentials up to approximately 5 V. DPF1S₃MN is electrochemically viable by fundamental Pt oxidation and graphite reduction.

Synthesis of DF1S₃MSO

DF1S₃MSO was obtained as byproduct of incomplete oxidation during the synthesis of DF1S₃MS according to the procedure mentioned. DF1S₃MSO was purified by distillation under vacuum at 40° C. at 0.1 Torr.

Synthesis of F1S₃MA

In this synthesis, 2 mol equivalents of dimethylallylamine is mixed with 1,1,3,3-tetramethyldisiloxane and a small amount of Karstedt's catalyst. The mixture is heated to 100° C. and left reacting overnight. Next day, the mixture was fluorinated using 0.67 mol equivalent of antimony trifluoride at 150° C. overnight with strong stirring. Next day, the solid was filtered off, and the product distilled under vacuum between 20-25° C. at 0.2 Torr to yield the desired product, F1S₃MA.

Synthesis of F1S₃MC

Allyl alcohol was silylated with hexamethyldisilazane, using a catalytic amount of aluminum dihydrogenphosphate at 80° C. overnight. The intermediate allyloxytrimethylsilane was distilled to purify it before the hydrosilylation. The hydrosilylation was done overnight with 1 mol equivalent of dimethylchlorosilane and a small amount of Karstedt's catalyst at 80° C. Next day, the mixture was fluorinated and hydrolyzed using 2 mol equivalent of aqueous hydrofluoric acid at room temperature with strong stirring to get the (3-hydroxypropyl)dimethylfluorosilane, which was distilled before the next step. The last intermediate was dissolved in hexane, 1 mol equivalent of trimethylamine was added, the mixture cooled in an ice bath and methyl chloroformate was added dropwise to the mixture, then it was left reacting overnight at room temperature. Next day the solid was filtered off, the solvent evaporated and the product distilled under vacuum between 28° C. at 0.2 Torr to yield the desired product, F1S₃MC.

F1S₃MC was synthesized to compare the electrochemical performance of commonly used carbonates to a silyl analog. The CV oxidation and reduction of F1S₃MC was shown to be suitable for electrochemical application. The synthesis is quite good, yielding F1S₃MC in >99.8% purity. F1S₃MC dissolved readily in 1M LiPF₆ at room temperature. It displayed acceptable cycling at 30° C. with good capacity. F1S₃MC also displayed good oxidation stability at potentials up to about 5 V. In CV, reduction showed two peaks in the first cycle (at 1.7 V and 0.6 V) and passivation in the second cycle.

Determination of the Electrochemical Stability of Organosilicon Materials:

Computational chemistry methods were used to calculate electrochemical properties of various organosilicon molecules. We used the GAMESS program developed by the Gordon research group at Iowa State University for the Density Function Theory (DFT) molecular orbital calculations. The HOMO (highest occupied molecular orbital) and LUMO (lowest unoccupied molecular orbital) energy levels, which correlate to the reduction and oxidation potentials of compounds, were calculated at the B3LYP/DZV level. The oxidative stability of electrolytes containing organosilicon solvents was determined using linear sweep voltammetry (LSV) or cyclic voltammetry (CV) in a 3-electrode cell. A platinum microelectrode was used as the working electrode with lithium metal as both the counter and reference electrode. The potential of the system was increased from the open circuit voltage (OCV) to 6 or 8V (vs. Li/Li⁺) at a scan rate of 10 mV/s. The resulting current density (mA/cm²) was recorded at each potential with a higher current indicating an oxidative reaction (i.e., lower oxidative stability). For the linear sweep voltammetry, 8V was used as a final potential to evaluate the fundamental oxidative stability of the material across a wider voltage range. For the cyclic voltammetry, 6V was used to evaluate the material across multiple scans under potentials more relevant to traditional battery applications. Multiple scans were conducted in the cyclic voltammetry experiments to determine the reversibility/irreversibility of any reactions observed.

The reductive stability of electrolytes containing organosilicon solvents was determined using linear sweep voltammetry (LSV) in a 3-electrode cell. A glassy carbon electrode was used as the working electrode with lithium metal as both the counter and reference electrode. The potential of the system was decreased from the open circuit voltage (OCV, typically 3V) to 0.1V (vs. Li/Li⁺) at a scan rate of 10 mV/s. The resulting current density (mA/cm²) was recorded at each potential with a greater current indicating a reduction reaction (i.e., lower reductive stability). Two scans were conducted to evaluate if the reductive processes were reversible or irreversible (i.e., passivating).

Electrochemical Stability of F1S₃MN:

Molecular orbital diagrams for F1S₃MN and F1S₃M2, not shown, reveal that the energy difference between the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO) is greater for F1S₃MN (9.07 eV) than for F1S₃M2 (8.20 eV). F1S₃MN also has a higher oxidation potential (−8.75 eV) than F1S₃M2 (−6.84 eV).

FIGS. 1A and 1B depict the oxidation stability of F1S₃MN with LiPF₆, LiBF₄, or LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). The oxidation stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s. FIG. 1B depicts a close-up of the same data shown in FIG. 1A. The F1S₃MN-LiPF₆ electrolyte exhibited the best oxidation stability, having a current density of 1 mA/cm² at 7.3 V compared to a current density of 1 mA/cm² at 6.8 V and 6.2 V for F1S₃MN-LiBF₄ and F1S₃MN-LiTFSI, respectively.

FIGS. 2A and 2B depict the reduction stability of F1S₃MN with LiPF₆, LiBF₄, or LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). The reduction stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s. FIGS. 2A and 2B are two separate scans. The F1S₃MN-LiPF₆ electrolyte exhibited the best reduction stability.

FIGS. 3A and 3B depict the oxidation stability of F1S₃MN or F1S₃M2 with 1M LiPF₆ in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). The oxidation stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s. FIG. 3B depicts a close-up of the same data shown in FIG. 3A. F1S₃MN demonstrated improved oxidation stability with respect to F1S₃M2.

FIG. 4 depicts the reduction stability of F1S₃MN or F1S₃M2 with 1M LiPF₆ compared to a carbonate control electrolyte with LiPF₆ in current density (mA/cm²) versus voltage (V vs. Li/Li⁺) in two separate scans. The reduction stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s. F1S₃MN demonstrated less resistance to reduction compared to F1S₃M2.

Determination of Thermal Stability of Neat Solvents & Formulated Electrolytes:

The thermal stability of both the neat organosilicon solvents and the electrolyte compositions were determined as follows: Approximately 0.75 mL of liquid sample was heated in a sealed cell under an argon purge. The Argon purge was carried to an atmospheric sampling mass spectrometer where any gas phase impurities and/or decomposition products can be detected at very low levels using electron impact mass spectrometry (EI-MS). The sample was held for 1 hour at pre-determined temperature levels that are relevant for battery applications (30, 55, 70, 100, 125, 150, 175, and 200° C.). The gas phase decomposition products were identified by comparing fragmentation patterns obtained from the EI-MS to NIST standards. Following the heating experiment (and detection/collection of all gas phase products), the remaining liquid sample was analyzed via NMR spectroscopy for a quantitative analysis of the extent of decomposition. Multiple nuclei were examined to fully analyze all components of the system, including the organosilicon solvent, any carbonate co-solvents, all additives, and the lithium salt (if present).

Thermal Stability of F1S₃MN:

FIGS. 5A and 5B depict the thermal stability of F1S₃MN with LiPF₆. F1S₃MN-LiPF₆ electrolyte (batch ZP815-01) was exposed to temperatures ranging from 30° C. to 175° C. and analyzed by electron impact mass spectrometry (EI-MS) and nuclear magnetic resonance spectroscopy (NMR) for gas and liquid decomposition products, respectively. The temperatures at which salient peaks appeared are annotated. F1S₃MN showed no significant gas and/or liquid phase decomposition up to 175° C. Me₂SiF₂ appeared at temperatures of 100-125° C. at 81 m/z, and MeSiF₃ appeared at temperatures of 150-175° C. at 85 m/z. However, the 81 m/z and 85 m/z peaks appeared inconsistently at 100-175° C. Furthermore, ¹H NMR analysis showed no decomposition after heating to 175° C. Therefore, F1S₃MN does not show consistent decomposition up to 175° C. FIG. 5A depicts a close-up of the same data shown in FIG. 5B.

FIG. 6 depicts the thermal stability of F1S₃M2 with LiPF₆. F1S₃M2-LiPF₆ electrolyte was exposed to temperatures ranging from 30° C. to 150° C. and analyzed by mass spectrometry for decomposition products. The temperatures at which salient peaks appeared are annotated. F1S₃M2 showed decomposition at temperatures ≥125° C. Decomposition products included Me₂SiF₂ and 1,4-dioxane. ¹H NMR analysis showed approximately 6% decomposition at 150° C. These results in combination with those discussed in relation to FIG. 5A and FIG. 5B indicate that F1S₃MN is more thermally stable than F1S₃M2.

FIG. 7 depicts the thermal stability of F1S₃MN with LiTFSI. F1S₃MN-LiTFSI electrolyte was exposed to temperatures ranging from 30° C. to 185° C. and analyzed by mass spectrometry for decomposition products. The temperatures at which salient peaks appeared are annotated. Gas phase peaks were observed at temperatures ≥150° C. Peaks at 117 and 102 matched patterns observed for F1S₃MN-LiBF₄ electrolyte and neat solvent (see FIGS. 8 and 9).

FIG. 8 depicts the thermal stability of F1S₃MN with LiBF₄. F1S₃MN-LiBF₄ electrolyte was exposed to temperatures ranging from 30° C. to 200° C. and analyzed by mass spectrometry for decomposition products. The temperatures at which salient peaks appeared are annotated. Gas phase peaks were observed at temperatures ≥175° C. Peaks at 117 and 102 matched patterns observed for neat solvent and F1S₃MN-LiTFSI electrolyte (see FIGS. 7 and 9). ¹H NMR analysis showed no fluorinated decomposition products and <0.5% of a non-fluorinated hydrolysis product.

FIG. 9 depicts the thermal stability of neat F1S₃MN. F1S₃MN electrolyte was exposed to temperatures ranging from 30° C. to 195° C. and analyzed by mass spectrometry for decomposition products. The temperatures at which salient peaks appeared are annotated. Gas phase peaks were observed at temperatures ≥150° C. At 150° C., Me₂SiF₂ was observed (96/81 m/z), but other peaks were not associated with this product. ¹H NMR analysis showed no fluorinated decomposition products and <0.5% hydrolysis.

The above data show that F1S₃MN is the most thermally stable OS solvent with LiPF₆.

Synthesis of DF1S₃MN

Commercial 3-cyanopropyldichloromethylsilane (CAS No. 1190-16-5; Sigma Aldrich, St. Louis, Mo., US) was fluorinated with ammonium bifluoride at room temperature. Cold hexane was then added to the mixture. The solid was filtered off and the solvent evaporated. Calcium oxide was added to the crude product. The solvent was distilled under vacuum between 35-45° C. at 0.4 Torr to yield the desired product in very high purity (˜99.8%) and approximately 90% yield.

Synthesis of DF1S₂MN

Acrylonitrile was mixed with N,N,N′,N′-tetramethylethylenediamine and copper (I) oxide in a flask and heated to 60° C. Dichloromethylsilane was then added dropwise and refluxed overnight. After cooling to room temperature, the mixture was distilled under vacuum (43° C., 0.2 Torr) to yield the dichloro intermediate (DC11S₂MN). The intermediate was fluorinated using 1.2 mol equivalents of ammonium hydrogen fluoride at room temperature or 1.2 mol equivalents of sodium hydrogen fluoride at 130° C. Dichloromethane was then added and the solid filtered off. The solvent was evaporated and the crude product was distilled under vacuum. Triethylamine and molecular sieves were added to the product and distilled under vacuum between 25-33° C. at 0.1 Torr to yield the desired product at extremely high purity (>99%) at approximately 75% yield.

Thermal Stability of DF1S₃MN:

FIG. 10 depicts the thermal stability of DF1S₃MN with LiPF₆. DF1S₃MN-LiPF₆ electrolyte (ZP990-01) was exposed to temperatures from 30° C. to 150° C. and analyzed by electron impact mass spectrometry (EI-MS) and nuclear magnetic resonance spectroscopy (NMR) for gas and liquid decomposition products, respectively. DF1S₃MN showed no significant gas and/or liquid phase decomposition up to 150° C.

Differential Scanning Calorimetry (DSC) Evaluation for Thermal Abuse Tolerance:

DSC measurements were conducted with F1S₃MN and carbonate based electrolytes in the presence of de-lithiated cathode materials to evaluate potential thermal abuse tolerance effects that could translate to safety advantages in a full cell format. Higher onset temperature, lower total heat output and lower peak heat output are all effects that suggest improved thermal abuse behavior in full format cells.

FIG. 11 depicts the thermal stability of F1S₃MN with LiPF₆ and various carbonate co-solvents and is compared to a carbonate control electrolyte with LiPF₆. Cells containing each electrolyte were charged to 4.25V and then disassembled. The lithium nickel cobalt aluminum oxide (NCA) cathode was rinsed with diethylene carbonate and allowed to dry. Each sample containing 5 mg of active material and 2 mg of fresh electrolyte was hermetically sealed into a stainless steel DSC pan. DSC scans at a rate of 2° C./min showed that the carbonate control electrolyte reacted at a much lower onset temperature than any of the organosilicon electrolyte blends. Additionally, the electrolyte where organosilicon is substituted for EMC has a much lower peak heat output than the control electrolyte.

Preparation of Electrolytes:

Blending of electrolytes is completed inside a moisture-free (<5 ppm) and oxygen-free (<20 ppm) argon glove box. All electrolyte components, including solvents, salts, and additives have been properly dried before blending and are stored in the glove box. Solvent moisture is monitored periodically by Karl Fischer measurement to ensure moisture levels are maintained at <20 ppm. Generally, solvents are weighed first into a separate vial and mixed until homogeneous. 70% of the solvent is added to a volumetric flask. Lithium (or other) salt is added slowly and stirred by magnetic stir bar until completed dissolved. Any other additives (i.e. VC, LiBOB) are then added slowly and stirred until the solution is homogeneous. The stir bar is removed and a portion of the remaining solvent is added to complete the volumetric requirement. The stir bar is placed back into the volumetric flask and the electrolyte is stirred until homogeneous. After blending is complete the electrolyte is dispensed into a dried vial or alternate container for storage.

Performance of F1S₃MN in Lithium Ion Cells:

FIG. 12 depicts the discharge capacity at 30° C. of cells containing various electrolyte solvents. Three different electrolyte solvents were tested in Lithium Ion cells over a series of cycles at different C-rates in a 2032-size coin cell assembly (assembly stack as in FIG. 13) containing a graphite anode, a lithium nickel cobalt aluminum oxide (NCA) cathode, and “2500”-type separator from Celgard, LLC (Charlotte, N.C.). The three electrolyte solvents were: (1) control EPA6 carbonate electrolyte comprising 1:1 by volume ethylene carbonate (EC) and diethyl carbonate (DEC) (triangles); (2) an F1S₃MN-based electrolyte comprising 79% F1S₃MN, 20% EC, 1 M LiPF₆, and solid electrolyte interphase (SEI)-forming additives (squares); and (3) an F1S₃M2-based electrolyte, comprising 79% F1S₃M2, 20% EC, 1 M LiPF₆, and SEI-forming additives (circles). As shown in FIG. 12, the F1S₃MN-based electrolyte is equivalent to EPA6 at the 4C rate.

FIG. 14 depicts the discharge capacity at 55° C. of cells containing the same electrolytes as shown in, and described for FIG. 12. The cells were assembled in the same manner and cycled at a C/2 rate. As shown in FIG. 14, the F1S₃MN-based solvent had improved cycling stability at 55° C. compared to both the carbonate control and the F1S₃M2-based electrolyte.

Performance of F1S₃MN and DF1S₂MN in Electrical Double-Layer Capacitors Cells:

Symmetric electrical double layer capacitors (EDLC) were assembled into CR2032 coin cells as depicted in FIG. 15. A glass fiber separator (AP40, Merck Millipore) was sandwiched between two pieces of AC cloth electrode, with 100 μL electrolyte added to the separator. Tetraethylammonium tetrafluoroborate (TEA-BF₄, Alfa Aesar, 99%) and tetrabutylphosphonium hexafluorophosphate (TBP-PF₆, Sigma Aldrich, ≥99.0%) were used as the salts. Organosilicon solvents of F1S₃MN (99.4%) and DF1S₂MN (99.8%) were made by Silatronix. Acetonitrile (AN, Sigma Aldrich, anhydrous, 99.8%) was used as a co-solvent.

Zorflex FM10 100% activated carbon (AC) cloth from Calgon carbon was used for both electrodes. FM10 has 1000-2000 m²/g surface area, 0.5 mm thickness, and 120 g/m² area density. The AC cloth was punched to 15 mm diameter discs, and used directly as electrodes without any binder or conductive additives.

The performance of EDLC cells was tested by cyclic voltammetry (CV) using a Biologic BMP300 potentiostat. The temperature as control in an oven with variation as +0.1° C. The cyclic voltammetry (CV) responses of the EDLC cells was conducted between 0 and 3 V at a scan rate of 10 mV/s. A normalized specific capacitance, C, was derived according to the following equation [1,2]:

$C = \frac{i}{mv}$ where i is the current, v is the scan rate, m is the mass of one electrode.

FIG. 16 shows the cyclic voltammograms of EDLC cells with OS electrolytes containing TEA-BF₄ salt. Electrolyte ZX1193 included 1.0M TEA-BF₄ dissolved in 70 volume percent DF1S₂MN and 30 volume percent acetonitrile. Electrolyte ZX1190 included 0.8M TEA-BF₄ dissolved into blended DF1S₂MN and acetonitrile solvents, 60:40 by volume. The EDLC cells with both electrolyte formulations showed the regular and symmetric features to the 0 horizontal axis, indicating a non-redox or faradic properties of the cell.

FIG. 17 shows the cyclic voltammograms of EDLC cells with ZX1170 electrolyte and ZX1184 electrolyte containing TBP-PF₆ salt. Electrolyte ZX1170 has 1.2M TBP-PF₆ dissolved into F1S₃MN, and electrolyte ZX1184 has 1.2M TBP-PF₆ dissolved into DF1S₂MN. The non-redox or faradic properties can also be observed from the EDLC cells with both electrolyte ZX1170 and ZX1184 formulations.

1ND1N Synthesis:

Scheme 16 depicts a synthesis scheme for 1ND1N. 1ND1N cannot be chemically dried with sodium (Na), calcium oxide (CaO), or calcium hydride (CaH₂).

Electrochemical Stability of 1ND1N:

The molecular orbital diagram for 1ND1N and 1ND1, not shown, reveal the energy difference between the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO) for 1ND1N is 7.88 eV (LUMO=0.21 eV; HOMO=−7.88 eV) and for 1ND1 is 8.36 eV (LUMO=1.63 eV; HOMO=−6.73 eV). 1ND1N has great oxidation stability but lower reduction resistance than 1ND1.

FIG. 18 depicts the oxidation stability of 1ND1N with 1M LiPF₆ or 1M LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). The oxidation stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s.

FIG. 19 depicts the reduction stability of 1ND1N with 1M LiPF₆ or 1M LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). The reduction stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s. Two separate scans for each electrolyte are shown.

FIGS. 20A and 20B depict current density (mA/cm²) versus voltage (V vs. Li/Li⁺) for cycling scans with 1ND1N and 1M LiPF₆ or 1M LiTFSI from 0 to 6 V and from 6 to 0 V. FIG. 20A depicts a first cycle. FIG. 20B depicts a second cycle.

FIGS. 21A and 21B depict the oxidation stability of F1S₃MN or 1ND1N with 1M LiPF₆ in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). The oxidation stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s. FIG. 21B depicts a close-up of the same data shown in FIG. 21A. The F1S₃MN-LiPF₆ electrolyte had a current density of 1 mA/cm² at 7.3 V, and the 1ND1N-LiPF₆ electrolyte had a current density of 1 mA/cm² at 7.2 V.

FIGS. 22A and 22B depict the oxidation stability of F1S₃MN or 1ND1N with 1M LiTFSI in current density (mA/cm²) versus voltage (V vs. Li/Li⁺). The oxidation stability was tested at room temperature with a working electrode as Pt, a counter electrode as Li, a reference electrode as Li/Li⁺, and a sweep rate of 10 mV/s. FIG. 22B depicts a close-up of the same data shown in FIG. 22A. The F1S₃MN-LiTFSI electrolyte had a current density of 1 mA/cm² at 6.2 V, and the 1ND1N-LiTFSI electrolyte had a current density of 1 mA/cm² at 6.5 V.

Thermal Stability of 1ND1N:

FIG. 23 depicts the thermal stability of neat 1ND1N. 1ND1N was exposed to temperatures ranging from 30° C. to 189° C. and analyzed by mass spectrometry for decomposition products. 1ND1N showed no liquid or gas phase decomposition products up to 189° C. ¹H NMR showed ˜%5 decomposition.

FIG. 24 depicts the thermal stability of 1ND1N with LiPF₆. 1ND1N-LiPF₆ electrolyte was exposed to temperatures ranging from 30° C. to 150° C. and analyzed by mass spectrometry for decomposition products. The temperatures at which salient peaks appeared are annotated. 1ND1N showed gas phase decomposition ≥70° C., but no vigorous reaction was observed up to 150° C. Me₂SiF₂ (81 m/z) (96 g/mol) and a peak at 52/53 m/z suspected as being acrylonitrile (53 g/mol) appeared at a temperatures of 125-150° C. No 1,4-dioxane gas was observed at 150° C. ¹H NMR analysis showed that 50.6% 1ND1N remained at 125° C. and 58% remained at 150° C. At 125° C., presence of 39.7% fluorinated product F1NM1N (vs. 2.3% in unheated sample, 1.6% Me₂SiF₂ (vs. 0% in unheated sample), and 2.95% hydrolysis (vs. 5.5% in unheated sample) was observed. At 150° C., presence of 41% fluorinated product F1NM1N (vs. 2.3% in unheated sample), 1.7% Me₂SiF₂ (vs. 0% in unheated sample), and 5.0% hydrolysis (vs. 5.5% in unheated sample) was observed.

To identify the peaks observed at 52/53 m/z upon heating 1ND1N-LiPF₆ at 125-150° C., the mass spectrum profile for heated 1ND1N-LiPF₆ was compared with the mass spectrum profiles of National Institute of Standards and Technology (NIST) standards for 2-propenenitrile and hydrogen cyanide. FIG. 25A depicts a close-up of the mass spectrum profile as described with respect to FIG. 24 from 24-30 m/z. FIG. 25B depicts a close-up of the mass spectrum profile as described with respect to FIG. 24 from 49-55 m/z. The temperatures at which salient peaks in FIGS. 25A and 25B appeared are annotated. The peaks at 51, 52, and 53 m/z in FIG. 25B indicate that acrylonitrile is likely present. The presence of HCN cannot be definitively confirmed or disconfirmed due to the presence of peaks at 26 and 27 m/z in the NIST spectra. The spectrum in FIG. 25A shows a greater peak intensity at 26 m/z compared to 27 m/z, which supports the presence of acrylonitrile. However, the magnitude of the peak at 27 m/z is greater than expected for acrylonitrile alone.

FIG. 26 depicts the thermal stability of 1ND1N with LiTFSI, vinylene carbonate (VC) and lithium bis(oxalato)borate (LiBOB). 1ND1N-LiTFSI—VC-LiBOB was exposed to temperatures ranging from 30° C. to 185° C. and analyzed by mass spectrometry for decomposition products. 1ND1N-LiTFSI—VC-LiBOB showed no gas phase decomposition products up to 185° C. ¹H NMR showed an increase in hydrolysis from 3% (in the unheated sample) to 18.7% (after heating), which was likely due to a delay before the NMR analysis was performed.

FIG. 27 depicts the thermal stability of 1ND1N with LiBF₄. 1ND1N-LiBF₄ was exposed to temperatures ranging from 30° C. to 125° C. and analyzed by mass spectrometry for decomposition products. The temperatures at which salient peaks appeared are annotated. Gas phase products evolved at ≥30° C. As expected, Me₂SiF₂ (81 m/z) (96 g/mol) was observed. No acrylonitrile was observed. ¹H NMR showed 3.7% hydrolysis and 34.2% fluorinated products (3 sets of peaks). ¹⁹F NMR showed that all F in the system was bonded to Si. No BF₄ remained. There was insufficient F to fully decompose 1ND1N (˜5M 1ND1N versus 4 M F).

While no acrylonitrile was observed by mass spectrometry in heated 1ND1N-LiBF₄ samples, it was observed in unheated control (70 ppm). This indicates 1ND1N is not stable with LiBF₄ at room temperature. NMR analysis revealed that heating does little to increase decomposition, as shown in the following table:

³H (MeSi peak) hydrolysis fluorination Before Heating 3% 43% After Heating 4% 34% Performance of 1ND1N in Cells:

FIG. 28 depicts the discharge capacity of cells containing various electrolytes at a variety of C-rates. The electrolyte solvents were: (1) 1ND1N; (2) 1ND1N with 20% ethylene carbonate (EC) co-solvent (1ND1N_EC); and (3) 1ND2 with 20% EC co-solvent (1ND2_EC). All formulations also contained SEI-forming additives and 1 M LiPF₆ salt. As shown in FIG. 28, 20% EC co-solvent improved the performance of 1ND1N. With 20% EC co-solvent, 1ND1N showed diminished performance compared to 1ND2 at all C-rates.

FIG. 29 depicts the discharge capacity of cells containing various other electrolyte solvents. The electrolyte solvents were: (1) 1ND1N with 20% EC co-solvent, 1 M LiPF₆ and SEI-forming additives (1ND1N-EC-LiPF₆, shown as 1ND1N_EC in FIG. 29); (2) 1ND1N with 20% EC co-solvent, 1 M LiTFSI and SEI-forming additives (1ND1N-EC-LiTFSI, shown as 1ND1N_T in FIG. 29); and (3) 1ND2 with 20% EC co-solvent, 1 M LiPF₆ and SEI-forming additives (1ND2-EC-LiPF₆, shown as CP597-07 in FIG. 29). The 1ND1N-EC-LiPF₆ combination and the 1ND1N-EC-LiTFSI combination showed performance comparable to the 1ND2-EC-LiPF₆ combination.

FIGS. 30A and 30B depict the discharge capacity of cells containing a 1ND1N-LiPF₆-based electrolyte or a 1ND1N-LiTFSI-based electrolyte, respectively, at a variety of C-rates. For each experiment, a CR2032 coin cell with a Saft America (Cockeysville, Md.) NCA cathode, a graphite anode, and a 2500 separator from Celgard, LLC (Charlotte, N.C.) was used. The cells were charged with a constant-current/constant-voltage (CCCV) procedure at C/5, C/2, 1C or 2C rates to 4.1 V. The cells were discharged each cycle to 3.0 V with a constant current at the same rate that they were charged. In FIG. 30A, the 1ND1N-LiPF₆-based electrolyte solution included 1 M LiPF₆ and 1ND1N (batch ZP780-01), and the charging/discharging was performed at 30° C. or 55° C. In FIG. 30B, the 1ND1N-LiTFSI-based electrolyte solution included 1 M LiTFSI and 1ND1N, batch (ZT781-01), and the charging/discharging was performed at 30° C., 55° C., or 70° C. As shown in FIGS. 30A and 38B, the 1ND1N-LiTFSI-based electrolyte displayed better rate capability than the 1ND1N-LiPF₆-based electrolyte.

Physical Properties of OS Solvents and Electrolyte Solutions:

Table 1, above, shows physical properties of selected organosilicon (OS) compounds (1S₃MN, F1S₃MN, F1S₃cMN, DF1S₃MN, DF1S₂MN, and F1S₃M2) as neat solvents and formulated electrolyte solutions. Table 2, above, shows physical properties of neat 1ND2, 1ND1, 1ND1N F1S₃MN, DPF1S₃MN, F1S₃MC, F1S₃ME, F1S₃MA, F1S₃MS, 1NMS, F1S₃M2, and F1S₃cMN and various electrolyte compositions containing them. In both tables, the conductivity has units of mS/cm, the viscosity has units of cP, and the flash point is in degrees Celsius.

Proton (¹H) NMR spectra taken in CDCl₃ for 1ND1N, 1ND1N, DF1S₂MN, DF1S₃MN, F1S₃cMN, and 1S₃MN are presented in FIGS. 31-36, respectively. For selected compounds containing a fluorine atom, ¹⁹F-NMR data were collected in CDCl₃ and DMSO-d₆. The results are tabulated below:

¹⁹F-NMR in CDCl₃

F1S₃MN −162.3 ppm, ¹J(¹⁹F,²⁹Si)=280 Hz

isoF1S₃MN −166.6 ppm, ¹J(¹⁹F,²⁹Si)=284 Hz

DF1S₃MN −135.3 ppm, ¹J(¹⁹F,²⁹Si)=296 Hz

TF1S₃MN −136.8 ppm, ¹J(¹⁹F,²⁹Si)=280 Hz

DF1S₂MN −135.2 ppm, ¹J(¹⁹F,²⁹Si)=296 Hz

¹⁹F-NMR in DMSO-d₆

F1S₃MN −159.2 ppm, ¹J(¹⁹F,²⁹Si)=279 Hz

Thermal Stability of OS Electrolyte Solutions:

FIGS. 37 and 38 depict the gas phase decomposition of F1S₃MC, F1S₃cMN, 1S₃DN DF1S₂MN, TF1S₂MN and TF1S₃MN with 1M LiPF₆. Each electrolyte was exposed to temperatures ranging from 30° C. to 175° C. (60 min at each step) and analyzed by electron impact mass spectrometry (EI-MS) and nuclear magnetic resonance spectroscopy (NMR) for gas and liquid decomposition products, respectively. No significant gas and/or liquid phase decomposition was noted up to 175° C.

CONCLUSIONS

F1S₃MN and 1ND1N are both suitable for use as electrolyte solvents in Li-ion batteries. F1S₃MN and DF1S₂MN have demonstrated function as electrolyte solvents in EDLC devices. F1S₃MN shows very high thermal stability (measured by ¹H NMR) with all salts tested. F1S₃MN shows the highest thermal stability of any OS with LiPF₆ (175° C.), with no observed decomposition. F1S₃MN does produce gas phase products as neat solvent, with LiBF₄, and with LiTFSI. These gas phase products can be attributed to low levels of F1S₃MN evaporation. F1S₃MN shows increased voltage stability (higher oxidation potential with wide window) compared to F1S₃M2. F1S₃MN provides equivalent performance as EPA6 up to a rate of 4 C. LiBOB has limited solubility in F1S₃MN (<0.03M) without co-solvent, but LiBOB solubility improves (>0.1M) with use of co-solvent (i.e. 20% EC). The decomposition products of F1S₃MN are Me₂SiF₂ and MeSiF₃, both of which are gases.

1ND1N shows no gas phase decomposition as a neat solvent or in combination with LiTFSI electrolyte up to 185-190° C. The combination of 1ND1N with LiTFSI electrolyte shows promise up to 70° C. and higher. 1ND1N with LiPF₆ is more thermally stable than either 1ND1 or 1ND2 with LiPF₆. It forms acrylonitrile above 125° C. Like other non-spacer compounds, 1ND1N reacts at room temperature with LiBF₄. However, there is insufficient F to fully decompose the 1ND1N, and it does not form acrylonitrile. The rate performance of 1ND1N is slightly lower than 1ND2.

F1S₃ME, DPF1S₃MN and F1S₃MC are all suitable for use as electrolyte solvents in Li-ion batteries. F1S₃MC, F1S₃cMN, 1S₃DN, DF1S₂MN, TF1S₂MN, and TF1S₃MN demonstrate thermal stability with LiPF₆ (175° C.), with no observed decomposition. 

What is claimed is:
 1. A compound selected from the group consisting of: (R)_(4-a)—Si-((Sp-Y)—Z_(b))_(a)  (Formula I) wherein: “a” is 1; “b” is 0 to 3; “Z,” which is absent when “b”=0, is selected from the group consisting of halogen, C₁₋₆ linear or branched alkyl, alkenyl, and alkynyl, and

where each “R” is independently selected from the group consisting of halogen, C₁₋₆ linear or branched alkyl, alkenyl, and alkynyl, provided that at least one R is fluorine; each “Sp” in Formulas I and II is independently selected from the group consisting of C₂ alkylenyl; and each “Y” in Formula I is


2. The compound of claim 1, wherein “b” is 1 and “Z” is selected from the group consisting of halogen, C₁₋₆ linear or branched alkyl, alkenyl, and alkynyl.
 3. An electrolyte composition comprising a compound as recited in Claim 1, in combination with a salt.
 4. The electrolyte composition of claim 3, wherein the salt is a lithium-containing salt.
 5. An electrochemical device comprising an electrolyte composition as recited in claim
 3. 